Hydrogen and oxygen combine to from `H_(2) O_(2) ` and `H_(2)O` containing `5.93%` and `11.2%` hydrogen respectively . The data illustrates :

Options

A. law of conseravtion of mass
B. law of constant proportion
C. law of reciparocal proporation
D. law of multiple proporetion

Answer

To solve the problem, we need to analyze the given information about hydrogen and oxygen combining to form two different compounds: hydrogen peroxide (H₂O₂) and water (H₂O). We will use the percentages of hydrogen in these compounds to illustrate the law of multiple proportions.

### Step-by-Step Solution:

1. **Identify the Compounds and Their Percentages**:
- The compounds formed are H₂O₂ and H₂O.
- The percentage of hydrogen in H₂O₂ is 5.93%.
- The percentage of hydrogen in H₂O is 11.2%.

2. **Determine the Mass of Hydrogen in Each Compound**:
- For H₂O₂:
- The molar mass of H₂O₂ = (2 × 1) + (2 × 16) = 34 g/mol.
- Mass of hydrogen in H₂O₂ = (2 g / 34 g) × 100 = 5.93%.
- For H₂O:
- The molar mass of H₂O = (2 × 1) + (16) = 18 g/mol.
- Mass of hydrogen in H₂O = (2 g / 18 g) × 100 = 11.2%.

3. **Calculate the Mass of Oxygen in Each Compound**:
- For H₂O₂:
- Mass of oxygen = 34 g - 2 g = 32 g.
- For H₂O:
- Mass of oxygen = 18 g - 2 g = 16 g.

4. **Establish the Ratio of Masses of Oxygen**:
- In H₂O₂, the ratio of hydrogen to oxygen is 2:32 or simplified to 1:16.
- In H₂O, the ratio of hydrogen to oxygen is 2:16 or simplified to 1:8.

5. **Compare the Ratios**:
- The mass of hydrogen remains constant (2 g) in both compounds.
- The mass of oxygen changes, illustrating a simple whole number ratio (16:8 or 2:1).

6. **Conclusion**:
- Since the mass of hydrogen is fixed and the mass of oxygen varies in a simple ratio, this scenario illustrates the law of multiple proportions.

### Final Answer:
The data illustrates the **law of multiple proportions**.